Formate

Short description: Salt or ester of formic acid

Formate

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Names
Preferred IUPAC name

Formate

Systematic IUPAC name

Methanoate

Other names

Formylate
Methylate
Isocarbonite
Carbonite(1-)
Hydrogencarboxylate
Metacarbonoate
Oxocarbinate
Oxomethyl oxide ion
Oxomethoxide

Identifiers

CAS Number

* 71-47-6 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 277 Y

MeSH | Formates

PubChem CID

* 283

UNII |

* 0YIW783RG1 Y

SMILES

* O=C[O-]

Properties

Chemical formula

| HCOO− or HCO−2
Molar mass | 45.017 g mol−1
Conjugate acid | Formic acid

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Infobox references

Tracking categories (test):

* SizeSet

Formate (IUPAC name: methanoate) is the conjugate base of formic acid. Formate is an anion (HCO−
2) or its derivatives such as ester of formic acid. The salts and esters are generally colorless.[1]

## Contents

* 1 Fundamentals
* 2 Biochemistry
* 3 Formate esters
* 4 Formate salts
* 5 Examples
* 6 References

## Fundamentals

When dissolved in water, formic acid converts to formate:

HCO
2H → HCO−
2 \+ H+

Formate is a planar anion. The two oxygen atoms are equivalent and bear a partial negative charge. The remaining C-H bond is not acidic.

## Biochemistry

Formate is a common C-1 source in living systems. It is formed from many precursors including choline, serine, and sarcosine. It provides a C-1 source in the biosynthesis of some nucleic acids. Formate (or formic acid) is invoked as a leaving group in the demethylation of some sterols.[2] These conversions are catalyzed by aromatase enzymes using O2 as the oxidant. Specific conversions include testosterone to estradiol and androstenedione to estrone.[3]

Formate is reversibly oxidized by the enzyme formate dehydrogenase from Desulfovibrio gigas:[4]

HCO−
2 → CO
2 \+ H+
\+ 2 e−

## Formate esters

Formate esters have the formula HCOOR (alternative way of writing formula ROC(O)H or RO2CH). Many form spontaneously when alcohols dissolve in formic acid.

The most important formate ester is methyl formate, which is produced as an intermediate en route to formic acid. Methanol and carbon monoxide react in the presence of a strong base, such as sodium methoxide:[1]

3OH + CO → HCOOCH

Hydrolysis of methyl formate gives formic acid and regenerates methanol:

HCOOCH
3 → HCOOH + CH
3OH

Formic acid is used for many applications in industry.

Formate esters often are fragrant or have distinctive odors. Compared to the more common acetate esters, formate esters are less commonly used commercially because they are less stable.[5] Ethyl formate is found in some confectionaries.[1]

## Formate salts

Formate salts have the formula M(O2CH)(H2O)x. Such salts are prone to decarboxylation. For example, hydrated nickel formate decarboxylates at about 200 °C with reduction of the Ni2+ to finely powdered nickel metal:

Ni(HCO

2(H
2O)
2 → Ni + 2 CO
2 \+ 2 H
2O + H

Such fine powders are useful as hydrogenation catalysts.[1]

## Examples

Copper(II) formate hydrate

* ethyl formate, CH3CH2(HCOO)
* sodium formate, Na(HCOO)
* potassium formate, K(HCOO)
* caesium formate, Cs(HCOO); see Caesium: Petroleum exploration
* methyl formate, CH3(HCOO)
* methyl chloroformate, CH3OCOCl
* triethyl orthoformate
* trimethyl orthoformate, C4H10O3
* phenyl formate HCOOC6H5
* amyl formate

## References

1. ↑ 1.0 1.1 1.2 1.3 Werner Reutemann and Heinz Kieczka "Formic Acid" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a12_013
2. ↑ Pietzke, Matthias; Meiser, Johannes; Vazquez, Alexei (2020). "Formate Metabolism in Health and Disease". Molecular Metabolism 33: 23–37. doi:10.1016/j.molmet.2019.05.012. PMID 31402327.
3. ↑ Lephart, E. D. (1996). "A Review of Brain Aromatase Cytochrome P450". Brain Res. Rev. 22 (1): 1–26. doi:10.1016/0165-0173(96)00002-1. PMID 8871783.
4. ↑ T. Reda, C. M. Plugge, N. J. Abram and J. Hirst, "Reversible interconversion of carbon dioxide and formate by an electroactive enzyme", PNAS 2008 105, 10654–10658. doi:10.1073/pnas.0801290105
5. ↑ Johannes Panten and Horst Surburg "Flavors and Fragrances, 2. Aliphatic Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2015, Wiley-VCH, Weinheim.doi:10.1002/14356007.t11_t01

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